A 10.8g sample of a gas has a volume of 5.25L at 25 degrees Celsius and 766mmHg.

If 2.3g of the same gas is added to this constant 5.25L volume and the temperature raised to 68 degrees Celsius, what is the new gas pressure?

Use PV = nRT and solve for n (from the first 10.8 g sample). Then

moles = n = grams/molar mass.
You know N and g, solve for molar mass.

Then convert 2.3 g to moles (moles = grams/molar mass), add to moles at the beginning, and use PV = nRT again to solve for P.

To find the new gas pressure, we can use the ideal gas law equation:

PV = nRT

Where:
P = Pressure
V = Volume
n = number of moles of gas
R = ideal gas constant
T = temperature in Kelvin

Let's first calculate the initial number of moles of gas using the given data.

Step 1: Convert the mass of the gas to moles.
Given:
Mass of gas = 10.8g
Molar mass of the gas = unknown

To find the molar mass of the gas, additional information is needed.

Step 2: Calculate the initial gas pressure using the ideal gas law.
Given:
Volume (V) = 5.25L
Temperature (T) = 25 degrees Celsius = 25 + 273.15 = 298.15K
Pressure (P) = 766mmHg

To convert the pressure from mmHg to atm, divide by 760:
Pressure (P) = 766mmHg / 760 = 1.009 atm

Step 3: Calculate the initial number of moles.

PV = nRT

n (number of moles) = PV / RT

Plugging in the values:
n = (1.009 atm) * (5.25 L) / [(0.0821 L*atm/(mol*K)) * (298.15 K)]

n (number of moles) ≈ 0.226 mol

Now, let's calculate the new gas pressure after 2.3g of the same gas is added and the temperature is raised to 68 degrees Celsius.

Step 4: Calculate the number of moles of the additional gas.
Given:
Mass of additional gas = 2.3g
Molar mass of the gas = unknown

Again, to find the molar mass, additional information is required.

Step 5: Calculate the total number of moles of gas.

Total number of moles = initial moles + additional moles
Total number of moles ≈ 0.226 mol + additional moles

Step 6: Calculate the new gas pressure using the ideal gas law.

Given:
Volume (V) = 5.25L
Temperature (T) = 68 degrees Celsius = 68 + 273.15 = 341.15K

Using PV = nRT:

P * 5.25 L = (0.226 mol + additional moles) * (0.0821 L*atm/(mol*K)) * 341.15 K
P = [(0.226 mol + additional moles) * (0.0821 L*atm/(mol*K)) * 341.15 K] / 5.25 L

From here, substitute "additional moles" with the number of moles of the additional gas calculated in Step 4.

This will give you the new gas pressure.

To find the new gas pressure, we can use the combined gas law equation:

(P₁V₁) / (n₁T₁) = (P₂V₂) / (n₂T₂)

Where:
P₁, P₂ are the initial and final pressures respectively.
V₁, V₂ are the initial and final volumes respectively.
n₁, n₂ are the initial and final amounts of gas respectively.
T₁, T₂ are the initial and final temperatures respectively.

Let's break down the given information:

Initial conditions:
Mass of the gas (n₁) = 10.8g
Volume (V₁) = 5.25L
Temperature (T₁) = 25 degrees Celsius = 298K (converted to Kelvin)
Pressure (P₁) = 766mmHg

Final conditions:
Mass of the gas added (n₂) = 2.3g
Volume (V₂) = 5.25L (constant volume)
Temperature (T₂) = 68 degrees Celsius = 341K (converted to Kelvin)
Pressure (P₂) = ?

Now, let's substitute the values into the combined gas law equation:

(P₁V₁) / (n₁T₁) = (P₂V₂) / (n₂T₂)

(766mmHg * 5.25L) / (10.8g * 298K) = (P₂ * 5.25L) / (2.3g * 341K)

Now, solve for P₂:

P₂ = (766mmHg * 5.25L * 2.3g * 341K) / (10.8g * 298K)

Using these values, we can calculate the new gas pressure.